Answer:
How much energy would be produced from the reaction of 2.40 moles hydrogen with 3.95 moles chlorine?
Explanation:
Given,
2.40 moles hydrogen reacts with 3.95 moles chlorine.
From the balanced chemical equation,
1mol. of H2 reacts with 1mol. of Cl2
then,
2.40mol. of H2 reacts with ----?mol of Cl2
So, the remaining moles of Cl2 is in excess.
The limiting reagent is--- H2.
1mol. of H2 releases --- 554kJ of energy
then,
2.40mol of H2 releases ---- ?
Answer is: deltaH =-1329.6kJ
<u>Answer:</u> The equilibrium constant for the given reaction is 0.8
<u>Explanation:</u>
Equilibrium constant is defined as the ratio of concentration of the products raised to the power its stoichiometric coefficients to the concentration of reactants raised to power its stoichiometric coefficient. It is represented as
For the general equation:
The equilibrium constant is represented as:
For the given chemical equation:
for this equation is given by:
Concentration at equilibrium of
Putting values in above equation, we get:
Hence, the equilibrium constant for the given chemical reaction is 0.8